A) \[Pt|{{H}_{2}}(g)|HCl(sol.n)||AgN{{O}_{3}}(sol.n)|Ag\]
B) \[Ag|AgCl(s)|KCl(sol.n)|HCl(sol.n),{{H}_{2}}(g)Pt\]
C) \[Pt|{{H}_{2}}(g)|KCl(sol.n)||AgCl(s)|Ag\]
D) \[Pt|{{H}_{2}}(g),HCl(sol.n)||AgCl(s)|Ag\]
Correct Answer: D
Solution :
The cell reaction is: \[\frac{1}{2}{{H}_{2}}(g)+AgCl(s){{H}^{+}}(aq)\] \[+C{{l}^{-}}(aq)+Ag(s)\] Obviously, here hydrogen is being oxidised and \[AgCl\] is getting reduced. Hence the correct cell representaiton will be: \[Pt|{{H}_{2}}(g),\,HCl(solution)||AgCl(s)|Ag\]You need to login to perform this action.
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